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Chemistry in Industry and Technology Chemistry in Industry and Technology

Chemistry in Industry and Technology - PowerPoint Presentation

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Chemistry in Industry and Technology - PPT Presentation

Option C The Blast Furnace This follows closely from IGCSE work If you cant remember the work you did at IGCSE then you need to revise You will learn about some different sources of iron and you will learn more detail about the chemical reactions that happen in a blast furnace ID: 174741

furnace iron blast oxide iron furnace oxide blast 2fe main reactions igcse learn ore fed compounds sources top carbon

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Slide1

Chemistry in Industry and Technology

Option CSlide2
Slide3

The Blast FurnaceSlide4

This follows closely from IGCSE work. If you can’t remember the work you did at IGCSE then you need to revise!

You will learn about some different sources of iron, and you will learn more detail about the chemical reactions that happen in a blast furnace.Slide5

Syllabus Statements

C1.1 State the main sources of iron.

C1.2 Describe the main reactions that occur in the blast furnace.Slide6

TuyereSlide7

The Iron Ore fed into the blast furnace may be a number of different compounds:

Haematite

Fe

2

O

3

(this is the one you learnt at IGCSE)

Magnetite

Fe3

O

4

Iron Pyrites

FeS

2

(Fool’s gold!)

FeS

2

must be converted to the oxide:

4FeS

2

+ 11O

2

 2Fe

2

O

3

+ 8SO

2Slide8

Coke is also fed in at the top.

This provides a source of carbon to reduce the iron oxide.

Fe

2

O

3

+ 3C

 2Fe + 3CO

This DOES happen to a small extent – but from IGCSE you know its not really that simple!Slide9

Most of the reduction is done by Carbon Monoxide CO.

C + O

2

 CO

2

CO

2

+ C  2COSlide10

This carbon monoxide then reduces the iron ore.

Either

Fe

2

O

3

+ 3CO

 2Fe + 3CO

2

Or

Fe

3

O

4

+ 4CO  3Fe + 4CO

2Slide11

Both these reactions are exothermic.

The iron produced is molten because of the high temperature.

(

Iron

melts at 1536 °C or 2797 °F (1811 K). It boils at 2862 °C or 5182 °F (3134 K

).)

It sinks to the bottom of the furnace where it can be “tapped”Slide12

There are 2 more possible reaction mechanisms that you need to learn:

If methane (“natural gas”) is blown into the furnace, then incomplete combustion can take place.

2CH

4

+ O

2

 2CO + 4H

2

Then either the CO can act as the reducing agent as before, or the H

2

can act as the reducing agent.

Write balanced equations for hydrogen reducing both the forms of iron oxide present.Slide13

Fe

3

O

4

+ 4H

2

 3Fe + 4H

2

O

Fe

2

O

3

+ 3 H

2

 2Fe + 3H

2

OSlide14

Getting rid of impurities

The iron ore fed into the blast furnace is NOT a pure chemical.

It contains impurities such as silicon (IV) oxide and aluminium oxide.

These come from the rocks which contain the iron compounds.Slide15

Relative abundance of elements in the Earth’s crust

Oxygen

46.6%

Silicon

27.7%

Aluminum

8.1%

Iron

5.0%

Calcium

3.6%

Potassium

2.6%

Magnesium

2.6% Slide16

The third raw material added at the top of the blast furnace is powdered limestone.

This decomposes at the high temperatures involved.

CaCO

3

CaO

+ CO

2

Calcium oxide is “quicklime”

Quicklime is very basic and reacts with the impurities we have mentioned.Slide17

CaO

+ SiO

2

 CaSiO

3

CaO

+ Al

2

O

3

 CaAl

2

O

4

Silicon oxide is a non-metal oxide and is therefore acidic.

Aluminium oxide is amphoteric!!Slide18

Both the compounds formed are liquids.

We call them “slag”

They float on top of the molten iron and can be removed through a second outlet.

They are used for roads and making cement.

Because they can be easily removed the blast furnace can be run continuously for a number of years

(good economics!).

Eventually the lining of the furnace breaks down and we have to let the whole thing cool down so we can replace it.Slide19

Reminder . . .

C1.1 State the main sources of iron.

C1.2 Describe the main reactions that occur in the blast furnace.Slide20

Summary . . .Slide21

TuyereSlide22